3. What mass of water would need to evaporate from your skin in order to dissipate 1.7X10 J of heat from your body? Given: H2O(1) H2O(g) Hvap = 40.7 kJ/mol or2261 J/g 4. How much energy (heat) is required to convert 52.0 gram of ice at -10.0C to steam at 100 °C? Given: Specific heat (ice): 2.09 J/g•C Htus = 6.02 kJ/mol or 334 J/g Specific heat (water): 4.18 J/g.C Hvap = 40.7 kJ/mol Specific heat (steam): 1.84 J/g-C 5. Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the expected value for the heat of sublimation of acetic acid?

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Chapter1: Chemical Foundations
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Answer number 3-5 I know you can answer 3 questions here  

1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to liquid
water at 60.0C. Given:
Specific heat (ice) = 2.1 J/g•C
Specific heat (water) = 4.18 J/g-C
Hfus = 6.0 kJ/mol or 334 J/g
2. Calculate the amount of heat needed to melt 2.00 kilogram of iron at its melting point (1,809 K), given
that: Hfus = 13.80 kJ/mol or 247 J/g
3. What mass of water would need to evaporate from your skin in order to dissipate 1.7X10$ J of heat from
your body? Given:
H2O(I) H2O(g) Hvap = 40.7 kJ/mol or2261 J/g
4. How much energy (heat) is required to convert 52.0 gram of ice at -10.0C to steam at
100 °C?
Given:
Specific heat (ice): 2.09 J/g•C Hrus = 6.02 kJ/mol or 334 J/g
Specific heat (water): 4.18 J/g•C Hvap = 40.7 kJ/mol
Specific heat (steam): 1.84 J/g-C
5. Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the
expected value for the heat of sublimation of acetic acid?
Transcribed Image Text:1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to liquid water at 60.0C. Given: Specific heat (ice) = 2.1 J/g•C Specific heat (water) = 4.18 J/g-C Hfus = 6.0 kJ/mol or 334 J/g 2. Calculate the amount of heat needed to melt 2.00 kilogram of iron at its melting point (1,809 K), given that: Hfus = 13.80 kJ/mol or 247 J/g 3. What mass of water would need to evaporate from your skin in order to dissipate 1.7X10$ J of heat from your body? Given: H2O(I) H2O(g) Hvap = 40.7 kJ/mol or2261 J/g 4. How much energy (heat) is required to convert 52.0 gram of ice at -10.0C to steam at 100 °C? Given: Specific heat (ice): 2.09 J/g•C Hrus = 6.02 kJ/mol or 334 J/g Specific heat (water): 4.18 J/g•C Hvap = 40.7 kJ/mol Specific heat (steam): 1.84 J/g-C 5. Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the expected value for the heat of sublimation of acetic acid?
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